What is the minimum amount of 1.75 m of HCL necessary to produce 28.5 L of H2 at stp?
EQUATION IS AS FOLLOWS:
Mg+2HCL->>MgCl2+H2
Is that an m or an M? I will assume you made a typo or didn't know any better and you meant M. Also, I assume you meant at STP.
28.5L H2 x (1 mole/22.4 L) = ?? moles H2.
moles HCl = ??moles H2 x (2 moles HCl/1 mole H2) = xx moles HCl.
M HCl = moles/liters HCl.
You know M and moles, solve for liters HCl
i did this and i still got the wrong answer. i got like 56.1 and the answer was 1.5. that's why i was lost
i did the same thing...the answer was 1.65
which is not what i got from the calculation
To find the minimum amount of 1.75 m of HCl necessary to produce 28.5 L of H2 at STP (Standard Temperature and Pressure), we need to use stoichiometry, which is the calculation of reactants and products in a chemical reaction.
The balanced chemical equation for the reaction between magnesium (Mg) and hydrochloric acid (HCl) is:
Mg + 2HCl -> MgCl2 + H2
According to the equation, 1 mole of magnesium reacts with 2 moles of hydrochloric acid to produce 1 mole of magnesium chloride and 1 mole of hydrogen gas.
To determine the amount of HCl needed to produce 28.5 L of H2, we can follow these steps:
Step 1: Convert the volume of H2 gas from liters to moles.
Since we are working with STP, 1 mole of any ideal gas occupies 22.4 liters at standard conditions. Therefore, we can calculate the number of moles of H2 using the following conversion:
28.5 L H2 * (1 mol H2 / 22.4 L H2) = 1.27 mol H2
Step 2: Apply mole ratios from the balanced equation.
According to the balanced equation, 1 mole of Mg reacts with 2 moles of HCl to produce 1 mole of H2. Therefore, the mole ratio between HCl and H2 is 2:1.
To find the amount of HCl needed to produce 1.27 moles of H2, we can set up the following proportional equation:
2 mol HCl / 1 mol H2 = x mol HCl / 1.27 mol H2
Simplifying the equation, we find:
x = (2 mol HCl * 1.27 mol H2) / 1 mol H2
x = 2.54 mol HCl
Step 3: Convert the amount of HCl from moles to volume.
The given concentration of HCl is 1.75 m (moles per liter). Therefore, to convert the HCl quantity from moles to liters, we use the following conversion:
2.54 mol HCl * (1 L HCl / 1.75 mol HCl) = 1.45 L HCl
Therefore, the minimum amount of 1.75 m of HCl necessary to produce 28.5 L of H2 at STP is approximately 1.45 L of HCl.