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What is the maximum mass of S8 that can be produced by combining 75 grams of each reactant?
The molar mass of S8 is 256 g/mol. To calculate the maximum mass of S8 that can be produced, first determine the limiting reactant by converting the masses of the reactants to moles. Then, use the stoichiometry of the reaction to find the mass of S8 produced from the limiting reactant.
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87.2 grams of glucose burned in 87.2 grams oxygen what is limiting reactant?
To determine the limiting reactant, you need to compare the amounts of reactants in terms of moles. First, convert the grams of glucose and oxygen into moles using their respective molar masses. Then, calculate the moles of products that can be formed from each reactant. The reactant that produces fewer moles of product will be the limiting reactant.
How much C2H4N2 could be expected from the reaction of 13.6 grams CO2 2.21 grams NH3 and 1.64 grams of CH4?
To determine the expected yield of C2H4N2 from the reaction of CO2, NH3, and CH4, we first need to identify the balanced chemical equation for the reaction. Assuming the reaction is balanced, we would calculate the moles of each reactant (CO2, NH3, and CH4) and identify the limiting reagent. The limiting reagent will dictate the maximum amount of C2H4N2 that can be produced. Since specific stoichiometric coefficients are not provided, you would need to perform these calculations based on the balanced equation to find the exact mass of C2H4N2 produced.
For each of the following precipitation reactions calculate how many grams of the first reactant are necessary to completely react with 56.5 g of the second reactant?
I'm happy to help, but I need the specific reactions in question in order to provide a detailed calculation. Once you provide the reactions, I can assist you in determining the grams of the first reactant needed to react with 56.5 g of the second reactant.
How many grams of iron can be made form 119 g of Fe2S3 and 12.7 g C?
To find how many grams of iron can be produced, calculate the molar mass of Fe2S3 and C, then use stoichiometry to determine the amount of Fe that can be produced. 1 mole of Fe2S3 produces 2 moles of Fe, and 1 mole of C produces 3 moles of Fe, so compare the moles of Fe produced from each reactant and choose the limiting reactant. Calculate the amount of Fe produced.
In a reaction 25 grams of reactant AB breaks down into 10 grams of product A and an unknown amount of product B. Using the law of conservation of mass how much does product B weigh?
According to the law of conservation of mass, the total mass of reactants must equal the total mass of products. In this case, the initial mass of reactant AB is 25 grams, and product A weighs 10 grams. Therefore, the mass of product B can be calculated as follows: 25 grams (mass of AB) - 10 grams (mass of A) = 15 grams. Thus, product B weighs 15 grams.
If 34.5 g of copper reacts with 70.2g of silver nitrate according to the following reaction what is the maximum number of grams of silver that can be produced answer?
To find the maximum number of grams of silver that can be produced, first calculate the moles of copper and silver nitrate using their respective molar masses. Then, determine the limiting reactant using the stoichiometry of the reaction. Finally, calculate the maximum number of grams of silver that can be produced by multiplying the moles of silver obtained from the limiting reactant by the molar mass of silver.
What is the maximum amount in grams of SO3 that can be produced by the reaction of 1.0g of S with 1.0g of O2 via the equation belowS O2-- SO3 not balanced?
To determine the maximum amount of SO3 that can be produced, we need to find the limiting reactant first. Given 1.0g of S and 1.0g of O2, we calculate the number of moles for each reactant. Then, we find the mole ratio from the unbalanced equation and determine which reactant is limiting. Finally, we can calculate the maximum amount of SO3 that can be produced from the limiting reactant.
What is the limiting reactant when 3.14g of nitrogen react with 2.79g of hydrogen to produce ammonia and how many grams of ammonia are produce?
To determine the limiting reactant, we need to find the moles of each reactant. Then, we calculate the amount of ammonia that can be produced from each reactant. Whichever reactant produces the least amount of ammonia is the limiting reactant. Finally, we calculate the grams of ammonia produced based on the limiting reactant.
How many grams of aluminum chloride could be produced from 34.0 grams of aluminum and 39.0 grams of chlorine gas?
To find the limiting reactant, we need to calculate the moles of each reactant. Then, use the stoichiometry of the balanced chemical equation to determine which reactant limits the amount of aluminum chloride that can be produced. Finally, calculate the mass of aluminum chloride produced based on the limiting reactant.
If 25.0 grams of potassium chlorate decomposes, how many grams of potassium chloride will be produced What is the limiting reactant?
I Don't knows Sorry
If 108 grams of Al are allowed to completely react with 318 grams of FeO how many grams of AlO and Fe will be produced?
To calculate the amount of AlO produced, you first need to determine the limiting reactant by converting the grams of Al and FeO to moles, then comparing their molar ratios. Once you find the limiting reactant, use stoichiometry to calculate the moles of AlO produced. Finally, convert the moles of AlO to grams. The same steps can be used to find the amount of Fe produced.
How many grams of silver chloride are formed when 10.0 g of silver nitrate reacts with 15.0 g of barium chloride?
To find the limiting reactant, we need to determine how many grams of silver chloride can be produced from each reactant and compare the results. Calculate the amount of silver chloride that can be produced from 10.0 g of silver nitrate. Calculate the amount of silver chloride that can be produced from 15.0 g of barium chloride. The reactant that produces the lesser amount of silver chloride will be the limiting reactant.
How many grams of aluminum chloride could be produced from 35.5g of aluminum and 39.0g of chlorine gas?
The balanced chemical equation for the reaction is: 2Al + 3Cl₂ → 2AlCl₃ Calculate the limiting reactant: Moles of Al: 35.5g / molar mass of Al Moles of Cl₂: 39.0g / molar mass of Cl₂ Determine which reactant gives the lower amount of AlCl₃ produced. Once you know the limiting reactant, use stoichiometry to calculate the grams of AlCl₃ produced.
Why is 160 grams of oxygen mass would be produced?
This question seems to be about the reactant side of a chemical equation. To calculate the mass of oxygen produced, you need to know the stoichiometry of the reaction. Without that information, it is not possible to determine why 160 grams of oxygen would be produced.
In a chemical reaction 300 grams of reactant A are combined with 100 grams of reactant B . both A and B reactant to completion. how much will the product weigh?
200
If there are 4 grams of reactant how many grams of product are produced by the chemical reaction?
The amount of product produced by a chemical reaction depends on the stoichiometry of the reaction, which is given by the coefficients in the balanced equation. Without the balanced equation or additional information, it is not possible to determine the exact amount of product produced from a specific amount of reactant. You would need to know the stoichiometry of the reaction to calculate the amount of product.
What is the maximum mass of aluminum chloride that can be formed when reacting 28.0g of aluminum with 33.0g of chlorine?
The formula of aluminium chloride is AlCl3. The atomic weight of aluminium is 27 and that of chlorine is 35.5. That means 35.5*3 grams of chlorine will combine with 27 grams of aluminium. So 33 grams of chlorine will combine with 8.37 grams of aluminium. The addition of both makes it 41.37 grams. In this reaction, the whole chlorine will be utilized and only part of the aluminium.
