Answer:
Q = 4019.4 J
Explanation:
Given data:
Mass of ice = 20.0 g
Initial temperature = -10°C
Final temperature = 89.0°C
Amount of heat required = ?
Solution:
specific heat capacity of ice is 2.03 J/g.°C
Formula:
Q = m.c. ΔT
Q = amount of heat absorbed or released
m = mass of given substance
c = specific heat capacity of substance
ΔT = change in temperature
ΔT = T2 - T1
ΔT = 89.0°C - (-10°C)
ΔT = 99°C
Q = 20.0 g ×2.03 J/g.°C × 99°C
Q = 4019.4 J
Answer:
Faster, and the substance will be a gas.
Explanation:
I'm quite not sure with it. But, I've tried my best. Since maybe the substance is liquid
Answer:
the formula that represents a polar molecule is NH3 the 3 is small and toward the bottom
<span>H2C2O4(aq) + 2OH- --> C2O4^2- + 2H2O(l)</span>