Answer:
D is the answer to this problem
Boyle Law says “the pressure of fixed amount of ideal gas which is at constant temperature is
inversely proportional to its volume".<span>
P = 1/V
<span>Where, P is pressure of the ideal gas and V is volume of the ideal gas.</span>
<span>For two situations, this law can be added as;
P</span>₁V₁ = P₂V₂<span>
</span><span>14 lb/in² x V₁ = 70 lb/in² x 500 mL</span><span>
</span><span>V₁ =
2500 mL</span><span>
Hence, the needed volume of atmospheric air = 2500
mL
<span>Here, we made two </span>assumptions. They are,
1. The
atmospheric air acts as ideal gas.
2.
Temperature is a constant.
<span>We didn't convert the units to SI units since
converting volume and pressure are products of two numbers, they will cut off. </span></span></span>
Answer:
Explanation:
Mole = no. Molecules/6.02×10^23
Mole = (2.35×10^24)/(6.02×10^23)
Mole = 3.9mole
<span>
all these are correct:
0 for Mg(s) and H in H2
</span><span>+1 for H in HCl
</span><span>-1 for Cl in HCl
</span>
<span>+2 for Mg in MgCl2
only the first statement is wrong</span>
