when the unstable compound ni3(s) decomposes, it produces nitrogen and iodine gases according to the…

when the unstable compound ni3(s) decomposes, it produces nitrogen and iodine gases according to the reaction 2ni3(s)→n2(g)+3i2(g). suppose 0.406 grams of ni3 decomposes. calculate the total number of moles of n2(g) and i2(g) produced. hint 0.00461 total moles incorrect. remember that n = m/m. attempts: 1 of 5 used save for later submit answer part 1 current attempt in progress

when the unstable compound ni3(s) decomposes, it produces nitrogen and iodine gases according to the reaction 2ni3(s)→n2(g)+3i2(g). suppose 0.406 grams of ni3 decomposes. calculate the total number of moles of n2(g) and i2(g) produced. hint 0.00461 total moles incorrect. remember that n = m/m. attempts: 1 of 5 used save for later submit answer part 1 current attempt in progress

Answer

Explanation:

Step1: Determine molar - mass of NI3

The molar - mass of NI3: N has a molar - mass of approximately 14.01 g/mol and I has a molar - mass of approximately 126.90 g/mol. So, (M_{NI_3}=14.01 + 3\times126.90=14.01 + 380.7=394.71\ g/mol).

Step2: Calculate moles of NI3

Given the mass of NI3 (m = 0.406\ g), using the formula (n=\frac{m}{M}), the number of moles of NI3, (n_{NI_3}=\frac{0.406\ g}{394.71\ g/mol}\approx0.00103\ mol).

Step3: Use stoichiometry

From the balanced chemical equation (2NI_3(s)\rightarrow N_2(g)+3I_2(g)), the mole ratio of (NI_3) to (N_2) is (2:1) and the mole ratio of (NI_3) to (I_2) is (2:3). The number of moles of (N_2) produced, (n_{N_2}=\frac{1}{2}n_{NI_3}=\frac{1}{2}\times0.00103\ mol = 0.000515\ mol). The number of moles of (I_2) produced, (n_{I_2}=\frac{3}{2}n_{NI_3}=\frac{3}{2}\times0.00103\ mol=0.001545\ mol).

Step4: Calculate total moles

The total number of moles of (N_2) and (I_2) produced is (n_{total}=n_{N_2}+n_{I_2}=0.000515\ mol + 0.001545\ mol=0.00206\ mol).

Answer:

0.00206