Final answer:
To find the ΔH when 3.50g of NO decomposes to its elements, convert the mass of NO to moles and use the mole ratio from the balanced equation to find the ΔH. for 1 mol NO into the equation, and multiply by the calculated value of x to find the ΔH when 3.50g of NO decomposes.
Step-by-step explanation:
The enthalpy change (ΔH) for 1 mole of NO(g) forming from its elements is given as 90.29 kJ. To find the ΔH when 3.50g of NO decomposes to its elements, we can use stoichiometry. First, we need to convert the mass of NO to moles using its molar mass. Then, we can use the mole ratio from the balanced equation to find the ΔH. Step 1: Convert mass of NO to moles: 3.50g NO x (1 mol NO / molar mass of NO) = x mol NO.
Step 2: Use the mole ratio from the balanced equation: x mol NO x (ΔH for 1 mol NO / 1 mol NO) = ΔH for 3.50g NO Substitute the given value for ΔH for 1 mol NO into the equation, and multiply by the calculated value of x to find the ΔH when 3.50g of NO decomposes.