Question

1. identify the limiting reactant when 1.00 g of si reacts with 0.75 g of n₂ in the following equation: 3si + 2n₂ → si₃n₄. options: n₂, n₄, si, si₃n₄. 2. multiple choice 1 point. what type of reaction is this an example of? ch₄(g) + 2o₂(g) → co₂(g) + 2h₂o(g). options: decomposition, combustion, composition, double replacement.

Explanation:

Question 1 (Identifying Limiting Reactant)

Step1: Calculate moles of Si

Molar mass of Si is \(28.09\space g/mol\). Moles of Si = \(\frac{1.00\space g}{28.09\space g/mol} \approx 0.0356\space mol\).

Step2: Calculate moles of \(N_2\)

Molar mass of \(N_2\) is \(28.02\space g/mol\). Moles of \(N_2\) = \(\frac{0.75\space g}{28.02\space g/mol} \approx 0.0268\space mol\).

Step3: Determine mole ratio from reaction

From \(3Si + 2N_2
ightarrow Si_3N_4\), the ratio of Si to \(N_2\) is \(3:2\).
For Si: \(\frac{0.0356}{3} \approx 0.0119\)
For \(N_2\): \(\frac{0.0268}{2} = 0.0134\)
Since \(0.0119 < 0.0134\), Si has a smaller ratio, so Si is the limiting reactant.

The reaction \(CH_4(g)+2O_2(g)
ightarrow CO_2(g)+2H_2O(g)\) involves a hydrocarbon (\(CH_4\)) reacting with oxygen (\(O_2\)) to produce carbon dioxide and water, which is the definition of a combustion reaction. Decomposition is breaking down a compound, composition is forming a compound from simpler substances, and double replacement involves ion exchange, none of which match here.

Answer:

Si (the option "Si")

Question 2 (Identifying Reaction Type)