We are tasked with determining the heat required to elevate the temperature of water from 85.0 ⁰F to 50.4 ⁰F.
To increase the temperature from 50.4 ⁰F to 85.0 ⁰F, a heat amount of 10.857 kJ is necessary.
The needed heat for the temperature increase can be calculated using the equation H = m×s×(t₂-t₁).
In this equation, H is the heat, s represents specific gravity at 4.184 J/g.⁰C, m is the mass of 135.0 g, t₁ (the initial temperature) is 50.4 ⁰F or 10.222 ⁰C, and t₂ (final temperature) stands at 85.0⁰F or 29.444 ⁰C.
After inputting these values, we find:
H = 135.0 g × 4.184 J/g.⁰C × (29.444 - 10.222) ⁰C
Simplifying gives us H = 10857.354 J or 10.857 kJ.
Thus, to elevate the temperature, 10857.354 J or 10.857 kJ of heat is necessary.
Missing question: A sample of O2 with a volume of 5.00 L at specified temperature and pressure contains 1.08x10^23 molecules. How many molecules would be present in each of the following under the same conditions? a) 5.00 L H2. b) 5.00 L CO2. Utilize Avogadro's Law: Equal volumes of all gases, at constant temperature and pressure, contain the same number of molecules. Hence, for both hydrogen and carbon dioxide—being gases—the number of molecules will equal the oxygen molecules, thus: a) N(H₂) = 1.08·10²³. b) N(CO₂) = 1.08·10²³.
