Answer:
90g of Ca(OH)2
Explanation:
2HCl + Ca(OH)2 —> CaCl2 + 2H20
Molar Mass of Ca(OH)2 = 40 + 2( 16 + 1) = 40 + 2(17) = 40 + 34 = 74g/mol
Molar Mass of CaCl2 = 40 + (2 x 3.5) = 40 + 71 = 111g/mol
From the equation,
74g of Ca(OH)2 produced 111g of CaCl2.
Therefore, Xg of Ca(OH)2 will produce 135g of CaCl2 i.e
Xg of Ca(OH)2 = (74 x 135) / 111 = 90g.
Therefore, 90g of Ca(OH)2 are required to produce 135g of CaCl2
The time measured by a stopwatch is not an exact number. The number is limited by the precision of the instrument (the stopwatch) and it migh have been 56.004 instead of 56.00, and the stopwatch cannot shoe that. So, this is not an exact number.
<span>the balanced equation for the reaction is as follows
2C</span>₄H₁₀ + 13O₂ ---> 8 CO₂ + 10H₂<span>O
stoichiometry of C</span>₄H₁₀ to O₂ <span>is 2:13
stoichiometry applies to the molar ratio of reactants and products. Avagadros law states that volume of gas is directly proportional to number of moles of gas when pressure and temperature are constant.
Therefore volume ratio of reactants is equal to molar ratio, volume ratio of C</span>₄H₁₀ to O₂<span> is 2:13
2 L of </span>C₄H₁₀ reacts with 13 L of O₂<span>
then 100 L of </span>C₄H₁₀<span> reacts with 13/2 x 100 = 650 L
therefore 650 L of O</span>₂<span> are required </span>