Answer:
There are formed 98.05 g of MnCl₂
Explanation:
The reaction is this one:
MnO₂ + 4 HCl → MnCl₂ + 2 H₂O + Cl₂
First of all, determinate moles. Divide mass /molar mass
150 g / 36.45 g/m = 4.11 moles of HCl
Ratio between HCl and MnCl₂ is 4:1
4 moles of HCl produce 1 mol of Chloride
4.11 moles of HCl 'll produce (4.11 . 1)/ 4 =1.03 moles of chloride
Molar mass . Moles = Mass
Molar Mass MnCl₂ = 95.2 g/m
95.2 g/m . 1.03 moles = 98.05 grams
They're totally unrelated. No matter how low or high the molecular weight, you can always use more or less of it.
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Answer:
0.14 M
Explanation:
To determinate the concentration of a new solution, we can use the equation below:
C1xV1 = C2xV2
Where C is the concentration, and V the volume, 1 represents the initial solution, and 2 the final one. So, first, the initial concentration is 1.50 M, the initial volume is 55.0 mL and the final volume is 278 mL
1.50x55.0 = C2x278
C2 = 0.30 M
The portion of 139 mL will be the same concentration because it wasn't diluted or evaporated. The final volume will be the volume of the initial solution plus the volume of water added, V2 = 139 + 155 = 294 mL
Then,
0.30x139 = C2x294
C2 = 0.14 M
Answer :
B
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