This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Welcome back Small — missed you this week. Let's solve question 4 parts (a)(ii), (a)(iii), (a)(iv), and (c)(ii)(I), (c)(ii)(II). Question 4(a)(ii): Write a balanced equation to show the complete combustion of butane. Step 1: Write the unbalanced equation for the complete combustion of butane (C_4H_10). C_4H_10 + O_2 CO_2 + H_2O Step 2: Balance the carbon atoms. C_4H_10 + O_2 4CO_2 + H_2O Step 3: Balance the hydrogen atoms. C_4H_10 + O_2 4CO_2 + 5H_2O Step 4: Balance the oxygen atoms. C_4H_10 + (13)/(2)O_2 4CO_2 + 5H_2O Step 5: Multiply the entire equation by 2 to remove the fraction. 2C_4H_10 + 13O_2 8CO_2 + 10H_2O Question 4(a)(iii): Calculate the molar mass of butane given that C=12 and H=1. Step 1: Identify the atomic masses and the chemical formula of butane (C_4H_10). Atomic mass of C = 12 g/mol Atomic mass of H = 1 g/mol Step 2: Calculate the molar mass. Molar mass of C_4H_10 = (4 × 12 g/mol) + (10 × 1 g/mol) Molar mass of C_4H_10 = 48 g/mol + 10 g/mol Molar mass of C_4H_10 = 58 g/mol The molar mass of butane is: 58 g/mol Question 4(a)(iv): How many moles are present in 11.6 g of Butane? Step 1: Use the formula for the number of moles. Number of moles = Mass