When burning magnesium ribbon is introduced into a jar of oxygen,it produces

On reaction of $38.1 \ g$ iodine and $28.4 \ g$ chlorine,a mixture of $ICl$ and $ICl_3$ is obtained. What will be the total number of moles after the reaction?

Balance the following chemical equation by choosing the correct option for the coefficients $x, y, p, q, r,$ and $s$.
$x KNO_3 + y C_{12}H_{22}O_{11} \longrightarrow p N_2 + q CO_2 + r H_2O + s K_2CO_3$

The number of moles of $H_2$ required to produce $10$ moles of $NH_3$ in the following reaction is:
$a H_{2(g)} + b NO_{2(g)} \longrightarrow c NH_{3(g)} + d H_2O_{(g)}$

Calculate the weight of $FeO$ produced from $6.7 \ g$ of $VO$ and $4.8 \ g$ of $Fe_2O_3$ using the reaction: $2VO + 3Fe_2O_3 \rightarrow 6FeO + V_2O_5$ $(V = 51, Fe = 56)$ (in $g$)

Assign $A, B, C, D$ from the given type of reaction.
$NaBr + AgNO_3 \longrightarrow AgBr \downarrow + NaNO_3$