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Does the compounds C2H2 and C6H6 have the same percent composition by mass?
It does not necessarily mean that. For example glucose (C6H12O6) and formaldehyde (CH2O) have the same percentages of elements by mass, but are two very difference compounds.
How many moles are in 0.244 grams of calcium carbide?
The chemical formula for Calcium Carbide is CaC2. So to find how many moles are in 0.244 grams of CaC2, you must first find the molar mass. Ca = 40.08 g/mol C = 12.01 g/mol Now that you have the molar mass, you just add it all together. Since there are two Carbon, you add it's mass twice. 40.08 + 12.01 + 12.01 = 64.1g Now you use Stoichiometry to convert the .244g to moles. 0.244g * (1 mol) / (64.1 g) = .00380655 mol The final answer would round to 0.00381 mol
How is an objects mass related to the upward force needed to overcome the pull of gravity?
Times the objects weight (In kilograms) by (approximately) 9.81 to get the objects mass on Earth. This figure, is the amount of Newtons (N) needed to overcome the pull of gravity. Example. A cat weighs 10Kg. 10X9.81 = 98.1N It would take 98.1N to lift this cat off the ground.
Why is a greater amount of force needed to accelerate a truck than a jeepney even if they are running with the same velocity?
The truck has a greater mass and therefore a greater amount of inertia to overcome. To accelerate a greater mass requires a greater force.
What is the speed it takes to move a 1 kilogram mass in one hour?
To know the speed of an object we need to know the distance the object travels and the time it takes. The object's mass is not needed. Since we do no know the distance in this case, we cannot solve to find its speed.
How many grams of water are needed to react with 492 g of calcium carbide?
Assuming pure calcium carbide: CaC2 + 2 H2O → C2H2 + Ca(OH)2 Molar mass of CaC2 = 64.1 Molar mass of water =18 ∴ no mol of CaC2 = 492/64.1=7.68mol ∴ no mol H2O =2*7.68=15.35mol ∴mass H2O = 15.35*18 = 276.3g of water
How many grams of C2H2 will be produced if 7 g of Ca(OH)2 are also produced in the following reaction CaC2 plus 2H2O C2H2 plus Ca(OH)2?
CaC2 + 2H2O ==> C2H2 + Ca(OH)2moles of C2H2 produced = moles of Ca(OH)2 produced (1:1 mole ratio is the stoichiometry)moles of Ca(OH)2 produced = 7 g x 1mol/74.1 g = 0.0945 molesmoles C2H2 = 0.0945 molesgrams C2H2 = 0.0945 moles x 26 g/mole = 2.46 grams = 2 grams to 1 sig fig
What mass of calcium bromide is needed to prepare 250 ml of a 2.50M?
The answer is 124,93 g (for the anhydrous CaBr2).
How much co2 is produced when 30000g of c2h2 burns completely?
2C2H2 + 5O2 ------------->2H2O + 4CO21 mole Of C2H2 = 26.04g, O2 = 32g, H2O = 44.01g, CO2 = 18.01g2moleC2H2 -------------> 4moleCO22x(26.04g) -------------> 4x(18.01g)52.08 g C2H2 ---------> 176.04 g CO230000g C2H2 ---------> ?? =176.04x30000g/52.08 =101405.53 gAnswer=101405.53 gram of CO2
How many grams of CoCl2 6H2O are needed to prepare 50.0ml of a 0.30M CoCl2 solution?
To determine the mass of CoCl2 6H2O to prepare a 0.30M solution in 50.0ml, we first calculate the molar mass of CoCl2 6H2O. The molar mass is 237.93 g/mol, so for a 0.30M solution in 50.0ml, we can use the formula: mass = molarity x volume (L) x molar mass. Therefore, the mass of CoCl2 6H2O needed is 3.57 grams.
How much water must be added to 425 g of formaldehyde to prepare a 40.0 percent by mass solution of formaldehyde?
To calculate the amount of water needed, first determine the mass of formaldehyde in the final solution. Since the solution is 40.0% formaldehyde by mass, the mass of formaldehyde is 40.0% of the final solution mass. Subtract the mass of formaldehyde in 425 g from this value to find the mass of water needed to prepare the solution.
What is the molecular formula of a compound that has a mass of 54 and an empirical formula of c2h2?
This is a hydrocarbon called Acetylene (IUPAC name : Ethyne). It contains two carbon atoms joined with a triple bond, and 2 hydrogen atoms connected to the two carbon atoms with a single bond. Its structure : H-C≡C-H
How many carbon atoms are contained in 84.3 g of ethyne (c2h2)?
3.90x10^24 atoms To arrive at an answer in units of carbon atoms, first we must cancel out the grams by diving 84.3g C2H2 by the molar mass of C2H2 (26.038g/mol). This molar mass is calculated by adding the masses of 2 carbon atoms (12.011g/mol) and 2 hydrogen atoms (1.008g/mol). This renders units of moles of ethyne. Next multiply by Avagadro's number (6.022x10^23 atoms/mol) to cancel the moles of ethyne and reach atoms of ethyne. Finally, because there are 2 carbon atoms in C2H2, multiply by 2 atoms Carbon/1 atom C2H2 to reach the final answer of 3.90x10^24 atoms of Carbon. This answer has been rounded to three significant figures because the lowest known value of significant figures throughout the calculations was three (84.3). The entire process is as follows: 84.3g C2H2 x (1 mol C2H2)/(26.038 g C2H2) x (6.022x10^23 atoms C2H2)/(1 mol C2H2) x (1 atoms C2H2)/(2 atom C) = 3.90x10^24 atoms C
What mass of KMnO4 is required to prepare 3.00 liters of a 0.05253 M solution of KMnO4?
To find the mass of KMnO4 needed, you can use the formula: mass = molarity x volume x molar mass. First, calculate the moles of KMnO4 using moles = molarity x volume. Then, multiply the moles by the molar mass of KMnO4 to find the mass needed.
How many grams of H20 can be produced by the reaction of 2.40mol c2 h2 with 7.40mol O2?
The equation for the reaction is 2 C2H2 + 5 O2 -> 4 CO2 + 2 H2O. Therefore, the minimum mole ratio of O2 to C2H2 to permit complete reaction is 5/2. The actual ratio present, 7.40/2.40 or about 3.08, is greater than this minimum; therefore, all the available C2H2 will react. The reaction equation shows that the number of moles of H2O produced is the same as the number of moles of C2H2 reacted. Therefore, 2.40 moles of H2O are produced. The gram molecular mass of H2O is about 18.015; therefore the mass of water produced is 43.2 grams, to the justified number of significant digits.
How many grams of K2SO4 would be needed to prepare 4.00 L of a 0.0510 M solution?
To calculate the grams of K2SO4 needed to prepare the solution, use the formula: (molarity) x (volume in liters) x (molar mass of K2SO4). First, calculate the moles of K2SO4 needed: 0.0510 mol/L x 4.00 L = 0.204 mol. Then, find the molar mass of K2SO4: 2*(39.10 g/mol) + 1*(32.07 g/mol) + 4*(16.00 g/mol) = 174.26 g/mol. Finally, multiply the moles by the molar mass: 0.204 mol x 174.26 g/mol ≈ 35.5 grams of K2SO4 are needed.
What mass of na2s2o3 5h2o is needed to prepare 500.00 ml of 0.1000 m na2s2o3?
Mol.Wt =248.17Molarity =( Wt/ Mol.Wt ) /No:of litres of solution0.1 =( Wt / 248.17) / 0.5Wt =0.1 *0.5*248.17Wt = 12.4085g in 500ml of solution.
