Honors Chem Chapter 5

Calculate the amount of heat in joules that 35.2 g of liquid water would need to absorb to increase in temperature by 10.0^oC.

• 1470 J

• 1820 J

• 737 J

• 656 J

Tags

NGSS.HS-PS3-4

Calculate the amount of heat in joules that 12.5 g of ethanol, C₂H₆O(l), would need to absorb to increase in temperature by 16.0^oC.

• 475 J

• 250 J

• 825 J

• 650 J

Tags

NGSS.HS-PS3-4

Calculate the amount of heat in joules that 56.8 g of aluminum, Al(s), would need to absorb to increase in temperature from 33^oC to 72^oC.

• 1987 J

• 1890 J

• 2050 J

• 2033 J

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

Calculate the amount of heat in joules that 56.8 g of copper, Cu(s), would need to absorb to increase in temperature from 33^oC to 72^oC.

• 853 J

• 995 J

• 288 J

• 880 J

Tags

NGSS.HS-PS3-4

What is the mass of a sample of gold that absorbs 650 J of energy and increases in temperature by 16^oC?

• 315 g

• 8.06 x 10⁴ g

• 5.24 g

• 3.18 x 10^-3 g

What is the mass of a sample of lead that absorbs 650 J of energy and increases in temperature by 16^oC?

• 312.5 g

• 8.00 x 10⁴ g

• 5.28 g

• 3.20 x 10^-3 g

A sample of iron increases in temperature from 100.0^oC to 275^oC by absorbing 5000.0 J. What is the mass of this sample of iron?

• 63.63 g

• 1.949 x 10⁶ g

• 12.83 g

• 3.062 x 10⁶ g

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

A sample of CO₂(g) increases in temperature from 50.0^oC to 75.0^oC by absorbing 4722 J. What is the mass of this sample of CO₂?

• 221 g

• 1.38 x 10⁵ g

• 161 g

• 4.15x 10⁵ g

Tags

NGSS.HS-PS3-4

What is the temperature change when 175 g He absorbs 6505 J of energy?

• 7.16^oC

• 2.18 x 10^{5 o}C

• 193^oC

• 48.2^oC

What is the temperature change when 615 g silicon, Si(s), absorbs 4568 J of energy?

• 10.4 ^oC

• 3.95 x 10^{6 o}C

• 5.31 ^oC

• 31.8 ^oC

Tags

NGSS.HS-PS3-4