how would i figure out this question?
assume that 5.60 L of H2 at STP reacts with CuO according to the equation: CuO+H2 yields Cu+H2O
a. how many moles of H2 react?
b. how many moles of Cu are produced?
c. how many grams of Cu are produced?
i have no clue what im doing! can you show me the steps on how to do this? thanks!
1. 1 mol of a gas occupies 22.4 L at STP. You have 5.60 L. So how many mols will that be?
2. Convert mols H2 to mols Cu using the coefficients in the balanced equation. Your prof may have called this dimensional analysis.
3. Convert mols Cu to grams Cu. grams = mols x molar mass.
Of course! I'll be happy to guide you through the steps to solve each part of the question.
a. To determine how many moles of H2 react, we need to use the ideal gas law at STP (Standard Temperature and Pressure). The STP conditions are 0 degrees Celsius (273.15 K) and 1 atm of pressure.
First, convert the given volume of H2 gas from liters to moles using the molar volume of a gas at STP, which is 22.41 L/mol:
5.60 L H2 × (1 mol H2/22.41 L H2) = 0.25 mol H2
Therefore, 0.25 moles of H2 react.
b. According to the balanced chemical equation, the stoichiometry tells us that 1 mole of H2 reacts with 1 mole of Cu. So, the same number of moles of Cu will be produced as the number of moles of H2 that react.
Hence, the number of moles of Cu produced will also be 0.25 moles.
c. To find the mass of Cu produced, we need to use the molar mass of Cu, which is 63.55 g/mol.
Multiply the number of moles of Cu produced by its molar mass:
0.25 mol Cu × 63.55 g/mol = 15.89 g Cu
Therefore, 15.89 grams of Cu are produced.
So, the answers are:
a. 0.25 moles of H2 react
b. 0.25 moles of Cu are produced
c. 15.89 grams of Cu are produced
Certainly! I'll guide you through each step to help you figure out the answers for each part of the question.
Step 1: Convert given volume of H2 gas (5.60 L) at STP to moles.
To convert from volume to moles, we can use the ideal gas law equation: PV = nRT. However, at Standard Temperature and Pressure (STP), the values of pressure (P) and temperature (T) are known: P = 1 atm and T = 273 K. Therefore, we can simplify the equation to:
V = nRT/P
Given V = 5.60 L, P = 1 atm, and T = 273 K, we can substitute these values into the equation to solve for n (the number of moles of H2).
Step 2: Determine the stoichiometry of the balanced chemical equation.
The balanced equation is CuO + H2 → Cu + H2O. From this equation, we can see that one mole of CuO reacts with one mole of H2 to produce one mole of Cu and one mole of H2O.
Step 3: Calculate the number of moles of H2 that react.
Since we know the volume of H2 at STP and have calculated the number of moles of H2 using the ideal gas law equation, we can say that the number of moles of H2 that react is equal to the number of moles of H2 we calculated in Step 1.
Step 4: Calculate the number of moles of Cu produced.
Since the stoichiometry of the balanced equation tells us that one mole of CuO reacts with one mole of H2 to produce one mole of Cu, the number of moles of Cu produced is equal to the number of moles of H2 that react.
Step 5: Calculate the mass of Cu produced.
To calculate the mass of Cu produced, we need to know the molar mass of Cu. The molar mass of Cu is 63.55 g/mol. Multiply the number of moles of Cu produced (from Step 4) by the molar mass of Cu to find the mass of Cu produced.
Now, let's put these steps into practice to find the answers to each part of the question:
a. To find the moles of H2 that react, use the ideal gas law equation: V = nRT/P. Substitute the given values and solve for n.
b. Since the stoichiometry of the balanced equation tells us that one mole of CuO reacts with one mole of H2 to produce one mole of Cu, the number of moles of Cu produced is equal to the number of moles of H2 that react.
c. Multiply the number of moles of Cu produced (from part b) by the molar mass of Cu to find the mass of Cu produced.
By following these steps, you'll be able to find the answers to each part of the question.