Consider the reaction of N aHCO3 with an acid, HA. How many grams of NaHCO3 are required to produce 1.25 g of CO2 ?

2.33g of NaHCO3

Explanation:

The balanced equation of the reaction is;

2NaHCO3  + 2HA --> 2CO2  +  2H2O + 2NaA

From the reaction above;

2 mol of NaHCO3 produces 2 mol of CO2

using mass = number of moles * molar mass

Mass = 2 * 84  = 164g of NaHCO3

Mass of CO2 = 2 * 44 = 88g of CO2

This means 164g of NaHCO3 produced 88g of CO2

How many grams of NaHCO3 would then produce 1.25g of CO2?

164 = 88

x = 1.25

upon solving for x;

x = 2.33g

d: the voltage of the secondary coil is less than that of the primary coil.

im not suree sorry if wrong