Stoichiometry and Thermochemistry Challenge

Consider the following unbalanced chemical equation: $$C_4H_{10} + O_2 \rightarrow CO_2 + H_2O$$ . Balance the equation and determine the coefficient of $$O_2$$ .

A reaction between 5.0 moles of $$N_2$$ and 10.0 moles of $$H_2$$ produces $$NH_3$$ . Identify the limiting reactant.

Calculate the amount of heat absorbed when 50.0 g of water is heated from 25°C to 75°C. (Specific heat capacity of water = 4.18 J/g°C)

Given the thermochemical equation: $$2H_2(g) + O_2(g) \rightarrow 2H_2O(l) \, \Delta H = -572 \, \text{kJ}$$ . How much heat is released when 4 moles of $$H_2$$ react completely?

Balance the following chemical equation: $$Fe + O_2 \rightarrow Fe_2O_3$$ . What is the coefficient of $$Fe$$ ?

In a reaction, 8.0 g of $$CH_4$$ reacts with 32.0 g of $$O_2$$ to form $$CO_2$$ and $$H_2O$$ . Determine the limiting reactant.

Calculate the heat change when 100 g of ice at 0°C melts to form water at 0°C. (Latent heat of fusion of ice = 334 J/g)

Analyze the following thermochemical equation: $$C(s) + O_2(g) \rightarrow CO_2(g) \, \Delta H = -393.5 \, \text{kJ}$$ . What is the enthalpy change when 2 moles of $$C$$ are burned?

Balance the chemical equation: $$C_3H_8 + O_2 \rightarrow CO_2 + H_2O$$ . What is the coefficient of $$CO_2$$ ?

A mixture of 10.0 g of $$H_2$$ and 50.0 g of $$O_2$$ is ignited to form water. Identify the limiting reactant.