How many liters of hydrogen gas are produced during an enthalpy change of
-50kJ, assuming STP conditions? 1L= 1kg
zn+ hno3 yields znn03 + 1/2 h2 +100kJ
-50 kj x (1mol h2/ 100kj) X (2.02g / 1 mol)
h2 )
= 1.01 g please help tried to get the answer but it it supposed to be 11.02 liters
To calculate the number of liters of hydrogen gas produced, we need to convert the given enthalpy change from kJ to moles of hydrogen gas. Then, we can use the ideal gas law to convert the moles of hydrogen gas to liters.
Given: -50 kJ
Step 1: Convert kJ to moles of hydrogen gas.
The enthalpy change is given in kJ, and the given chemical equation states that 100 kJ of energy is released when 1 mole of hydrogen gas is produced. So, we can set up a proportion:
-50 kJ * (1 mol H2 / 100 kJ) = -0.5 mol H2
Step 2: Convert moles of hydrogen gas to grams.
The molar mass of hydrogen gas (H2) is approximately 2.02 g/mol. We can use this information to convert moles to grams:
-0.5 mol H2 * (2.02 g / 1 mol H2) = -1.01 g H2
Note: The negative sign signifies that energy is released in the reaction.
Step 3: Convert grams of hydrogen gas to liters, assuming STP conditions.
The ideal gas law allows us to convert grams to moles, and moles to volume in liters at standard temperature and pressure (STP), which is 1 mole of any gas occupies a volume of 22.4 liters.
-1.01 g H2 * (1 mol H2 / 2.02 g) * (22.4 L / 1 mol H2) = -11.08 L H2
Note: We include the negative sign here because the enthalpy change is negative, indicating that the reaction releases energy.
Therefore, the correct answer is approximately -11.08 liters of hydrogen gas produced.