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Novay_Z [31]
3 years ago
7

Bill leaves his 60 W desk lamp on every day, including weekends, for eight hours. After one month (30 days), how much total ener

gy has been used by the lamp? Round your answer to the nearest whole number.
Physics
2 answers:
PolarNik [594]3 years ago
8 0
First multiply the 30 days by 8 hours to get 240, then take that number and multiply it by 60 W to get the final  answer of 14400. 
hope this is correct, I'm learning it too
Nana76 [90]3 years ago
8 0

The answer is 14 on edge

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During an isothermal process, 10 j of heat is removed from an ideal gas. What is the work done by the gas in the process?
Black_prince [1.1K]

The work done in the isothermal process is 10 joule.

We need to know about the isotherm process to solve this problem. The isotherm process can be described as a process where the initial temperature system will be the same as the final temperature. Hence, the internal energy change will be zero.

ΔU = 0

Hence,

ΔU = Q - W

0 = Q - W

Q = W

It means that the heat transferred is the same as the work done.

From the question above, we know that the heat transferred is 10 joule. Thus, the work done in the isothermal process is 10 joule.

Find more on isothermal at: brainly.com/question/17097259

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2 years ago
How much heat does it take to raise a<br> cup of water (2.34 x 10-4 m3) from<br> 15.0 °C to 75.0 °C?
Allisa [31]

Answer:58600

Explanation:

Trust me it’s correct.

8 0
3 years ago
A brick sliding across a smooth floor has a coefficient of static friction of s=0.23 and a coefficient of kinetic friction of k=
pantera1 [17]

Answer:

0.029325

Explanation:

0.23x0.15=0.0345

0.0345x0.85=0.029325

4 0
1 year ago
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Does every light source emit only one type of light?
blsea [12.9K]

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3 0
2 years ago
A 250. mL sample of gas at 1.00 atm and 20.0°C has the temperature increased to 40.0°C and the volume increased to 500. mL. What
ladessa [460]

Answer:

New pressure is 0.534 atm

Explanation:

Given:

Initial volume of the gas, V₁ = 250 mL

Initial pressure of the gas, P₁ = 1.00 atm

Initial temperature of the gas, T₁ = 20° C = 293 K

Final volume of the gas, V₂ = 500 mL

Final pressure of the gas = P₂

Final temperature of the gas, T₁ = 40° C = 313 K

now,

we know for a gas

PV = nRT

where,

n is the moles

R is the ideal gas constant

also, for a constant gas

we have

(P₁V₁/T₁) = (P₂V₂/T₂)

on substituting the values in the above equation, we get

(1.00 × 250)/293 = (P₂ × 500)/313

or

P₂ = 0.534 atm

Hence, the <u>new pressure is 0.534 atm</u>

5 0
3 years ago
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