The answer to this question B (10+10)/(5-3)
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<u>Answer:</u> The enthalpy of the reaction for given amount of ammonia will be -3431.3 kJ.
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
<u>For ammonia:</u>
Given mass of ammonia =
Molar mass of ammonia = 17 g/mol
Putting values in above equation, we get:
We are given:
Moles of ammonia = 74.11 moles
For the given chemical reaction:
By Stoichiometry of the reaction:
If 2 moles of ammonia produces -92.6 kJ of energy.
Then, 74.11 moles of ammonia will produce = of energy.
Thus, the enthalpy of the reaction for given amount of ammonia will be -3431.3 kJ.
From the equation,
4 mole of lithium produces 2 mole of lithium oxide
4.37 mol of lithium produces (4.37÷4)x2 mol of lithium oxide
Answer:
The volume of the sample of the gas is found to be 12.90 L.
Explanation:
Given pressure of the gas = P = 1.10 atm
Number of moles of gas = n = 0.6000 mole
Temperature = T = 288.15 K
Assuming the volume of the gas to be V liters
The ideal gas equation is shown below
Volume occupied by gas = 12.90 L