You are given
200 grams of H2O(s) at an initial temperature of 0°C. you are also given the
final temperature of water after heating at 65°C. You are required to get the
total amount of heat to melt the sample. The specific heat capacity, cp, of
water is 4.186 J/g-°C. Let us say that T1 = 0°C and T2 = 65°C. The equation for
heat, Q, is
Q = m(cp)(T2-T1)
Q = 200g(4.186
J/g-°C )(65°C - 0°C)
<u>Q =
54,418J</u>
Answer:
126.73 mL
Explanation:
The total pressure of the gas mixture is the sum of the vapor pressure of its constituents. So, the vapor pressure of N₂O(p) can be calculated:
750 = 18.85 + p
p = 750 - 18.85
p = 731.15 torr
It means that for 731.15 torr, N₂O occupied 130 mL. For the general gas equation, we know that

Where <em>p</em> is the pressure, <em>V</em> is the volume, <em>T</em> is the temperature, 1 is the initial state, and 2 the final state. For the same temperatue (21ºC), the equation results on Boyle's law:
p1V1 = p2V2, so:
731.15x130 = 750xV2
750V2 = 95049.5
V2 = 126.73 mL
Answer:
is this a T or F question? if so then T
Explanation:
The percent yield formula is % yield= (actual yield/theoretical yield) x 100
34.0g/50.0g= .68 x 100 = 68.0% (theres three sig. figs.)