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H2 Cl2 HCi?
The balanced equation is H2+ Cl2 --> 2HCl That is with a lowercase L, not an i.
What is the volume in L of HCL gas required to react with excess Ca to produce 11.4L of hydrogen gas at 1.62atm and 62 degrees C?
Double of 11.4 L H2, so 22.8 L HCl (at the same p and T) because 1 mol H2 is made out of 2 mol HCl according to:2HCl + 2Ca --> H2 + CaCl2
Is a H2 or hydrogen gas?
Hydrogen is a gas. H2 is the description of its molecular structure (2 hydrogen atoms bound together).
What is the gas formed when Mg reacted with sulfuric acid?
Mg + H2SO4 -> MgSO4 + H2 Hydrogen gas.
What volume of HCl gas is required to react with excess magnesium metal to produce 6.82 L of hydrogen gas at 2.19 ATM and 35 degrees C?
Balanced equation first. Mg + 2HCl >> MgCl2 + H2 ( use PV = nRT to find moles H2 ) ( C to K ) (1atm)(6.82L) =n(0.08206Latm/molK)(308.15K) = 0.2697 moles H2 ( drive back against HCL to find those moles ) 0.2697 moles H2 (2moles HCl/1mole H2) = 0.5394 moles HCl ( conditions remain the same, so use PV = nRT to find volume HCl ) (1atm)(Vol) = (0.5394 moles HCl)(0.08206Latm/molK)(308.15K) = 13.6 Liters HCl gas required ( may be faster way, but it is many years since I have done any chemistry )
How many grams of water form when 1.24L of H2 gas at STP reacts with O2?
When 1.24 L of H2 gas reacts with O2 at STP, the mole ratio between H2 and H2O is 2:2. This means that for every 1 mole of H2 gas reacting, 1 mole of water is formed. Using the ideal gas law, you can calculate the number of moles of H2 gas reacting, and then use the mole ratio to determine the number of moles of water formed. Finally, you can convert moles of water to grams using the molar mass of water.
Formula hydrogen gas?
Its H2
What is the product of H2?
The product of H2 is hydrogen gas (H2) composed of diatomic molecules.
What happens to h2 O when you remove oxygen?
It becomes the diatomic gas H2. Hydrogen gas.
H2 Cl2 HCi?
The balanced equation is H2+ Cl2 --> 2HCl That is with a lowercase L, not an i.
What is the volume in L of HCL gas required to react with excess Ca to produce 11.4L of hydrogen gas at 1.62atm and 62 degrees C?
Double of 11.4 L H2, so 22.8 L HCl (at the same p and T) because 1 mol H2 is made out of 2 mol HCl according to:2HCl + 2Ca --> H2 + CaCl2
Find the number of moles of h2 in 1420mL H2 gas?
To find the number of moles of H2 gas in 1420 mL, you need to use the ideal gas law. Given that the molar volume of gas at STP is approximately 22.4 L, you can convert 1420 mL to liters (1420 mL = 1.42 L) and then calculate the number of moles using the formula n = V/22.4, where n is the number of moles and V is the volume in liters.
How many liters of ammonia gas can be formed from 13.7 L of hydrogen gas at 93.0 C and a pressure of 40.0kPa?
At a constant temperature and pressure a mole of any gas has the same volume. So all you need to know to answer this question is that there are two atoms of hydrogen in a molecule of hydrogen gas and three atoms of hydrogen in a molecule of ammonia gas. 13.7 L * 2/3 = 9.13 L. You can check this by plugging the values into the ideal gas equation, pV = nRT (look on Wikipedia for "Ideal gas law")
Is a H2 or hydrogen gas?
Hydrogen is a gas. H2 is the description of its molecular structure (2 hydrogen atoms bound together).
What is the balance equation for hydrogen gas and iodine gas?
The balanced equation for the reaction between hydrogen gas (H2) and iodine gas (I2) to form hydrogen iodide gas (HI) is: H2 + I2 → 2HI
Why ammonia doesnt behave as an ideal gas?
NH3, as in Ammonia, like all real gases, are not ideal. Ideal gases follow the ideal gas laws, but ammonia does not adhere to a few of them. First of all, the volume of its molecules in a container is not negliggible. Next, NH3 molecules have intermolecular hydrogen bonding, which is a strong intermolecular bond. Thus, the forces of attaction between molecules is not neglible. All real gases have a certain degree of an ideal gas, but no real gas is actually ideal, with H2 being the closest to ideal.
How you Find the number of liters of hydrogen gas in 20 g of hydrogen at STP?
First find moles hydrogen gas. 20 grams H2 (1 mole H2/2.016 grams) = 9.921 moles H2 Now, the ideal gas equation. PV = nRT (1 atm)(volume L) = (9.921 moles H2)(0.08206 L*atm/mol*K)(298.15 K) Volume of hydrogen gas = 243 Liters ----------------------------------------------------
