All categories

3 years ago

The specific heat of aluminum is 0.90 J/gC . How much heat is given off when 25 grams of aluminum is cooled from 55 C to 25 C?

Physics

1 answer:

sp2606 [1]3 years ago

8 0

Answer:

2. How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22°C to 55°C, if the specific heat of aluminum is 0.90 J/gºC? c=0.90J/g. 9 (2 sigs.)

Explanation:

You might be interested in

A risk-free, zero-coupon bond with a $5000 face value has ten years to maturity. The bond currently trades at $3650. What is the

PtichkaEL [24]

Answer:

The Yield to Maturity of the bond is YTM = 3.20%

Explanation:

Mathematically the Yield to Maturity of the bond YTM is as follows

$YTM = \frac{C + \frac{F-P}{n} }{\frac{F+P}{2} }$

Where C is the amount of payment to be made = $0

P is the price i.e the present value =$3650

F is the face value of the bond=$5000

n is the year of maturity of the bond = 10 years

$YTM = \frac{0+\frac{5000-3650}{10} }{\frac{5000+3650}{2} } * \frac{100}{1}$

$=3.20$ %

5 0

3 years ago

What is the minimum energy required to lift an object weighing 200 Newtons at a height of 20 meters?

lakkis [162]

Work = force x distance

200 Newtons x 20 meters

= 4,000 Joules

4 0

3 years ago

Explain why a Chef in a very busy restaurant would prefer a copper pot over an aluminum pot. A) The copper pot would heat faster

stellarik [79]

A would be the answer

5 0

3 years ago

Read 2 more answers

The diameter of a copper atom is approximately 2.28e-10 m. The massof one mole of copper is 64 grams. Assume that the atoms area

KIM [24]

1) Mass of one copper atom: $1.063\cdot 10^{-22} kg$

2) There are $9.33\cdot 10^{24}$ atoms in the cube

3) Mass of the cubical block: 992 kg

Explanation:

We are told here that the mass of one mole of copper is

$M=64 g$

for

$n=1 mol$ (number of moles)

We also know that the number of atoms inside 1 mole of substance is equal to Avogadro number:

$N_A = 6.022\cdot 10^{23}$

This means that $N_A$ atoms of copper have a mass of M = 64 g. Therefore, we can find the mass of one copper atom by dividing the total mass by the avogadro number:

$m=\frac{M}{N_A}=\frac{64}{6.022\cdot 10^{23}}=1.063\cdot 10^{-22} kg$

We are told that the diameter of a copper atom is

$d=2.28\cdot 10^{-10} m$

We can assume that the atoms are arranged in a cube, and that they are all attached to each other; so the side of the cube can be written as size of one atom multiplied by the number of atom per side:

$L=Nd$