A student weighs out 0. 0422 g of magnesium metal. The magnesium metal is reacted with excess hydrochloric acid to produce hydro
1 answer:
The value of r is 0.0868 and the error percentage is 5.78%.
- The student weights 0.0422 grams of magnesium; thus, we may deduce that the magnesium he used is the mass of the magnesium over the additional mass, which is 0.024422.
- That is roughly equal to 0.001758.
- It also asserts that too much hydrochloric acid can react with magnesium, releasing hydrogen gas as a result.
- A sample of hydrogen gas is collected over water in a meter at a volume of 43.9 cc and a maximum pressure of 22 cc.
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Answer:
3.67 mol Cl
Explanation:
We need to convert g of Cl 2 to moles of Cl. First we divide 130 gCl2 by the molar mass (70.90 gCl2/mol) to find out how many moles of Cl2 do we have.
130 gCl2 x = 1.83 mol Cl2
Then we need to convert 1.83 mol de Cl2 to moles of Cl. We have 2 moles of Cl in every Cl2 molecule so we just need to multiply by 2.
1.83 molCl2 x = 3.67 molCl
<u>Answer:</u> The concentration of solution is 0.342 M
<u>Explanation:</u>
To calculate the molarity of solution, we use the equation:
We are given:
Mass of solute (Sodium chloride) = 15 g
Molar mass of sodium chloride = 58.5 g/mol
Volume of solution = 750 mL
Putting values in above equation, we get:
Hence, the concentration of solution is 0.342 M