What structural units make up network solids

An object with a mass of 3.2kg has a force of 16.3 newtons to the right and 6.7 newtons to the left applied to it. What is the r

Pepsi [2]

Answer:

3m/s²

Explanation:

Given parameters:

Mass of object = 3.2kg

Force to the right = 16.3N

Force to the left = 6.7N

Unknown:

Acceleration of the object = ?

Solution:

To solve this problem, we use newtons second law of motion;

Net force = mass x acceleration

Net force on object = Force to the right - Force to the left

Net force = 16.3N - 6.7N = 9.6N

So;

9.6 = 3.2 x a

a = $\frac{9.6}{3.2}$ = 3m/s²

7 0

2 years ago

Explain why food chains do not tend to exceed four links.

Softa [21]

Energy is "lost" at each trophic level when you go up the chain. Typically there are fewer organisms at higher trophic levels.

Hope this helps!

3 0

3 years ago

A train travels 65 km in three hours and then 52 km in two hours. What is its average speed?

Darya [45]

the average speed is 23.4 km per hour cause it is total distance over total time equal to average speed

5 0

3 years ago

A flask contains 6g hydrogen gas and 64 g oxygen at rtp the partial pressure of hydrogen gas in the flask of the total pressure

Alex

Answer:

B.3/5p

Explanation:

For this question, we have to remember "Dalton's Law of Partial Pressures". This law says that the pressure of the mixture would be equal to the sum of the partial pressure of each gas.

Additionally, we have a proportional relationship between moles and pressure. In other words, more moles indicate more pressure and vice-versa.

$P_i=P_t_o_t_a_l*X_i$

Where:

$P_i$ =Partial pressure

$P_t_o_t_a_l$ =Total pressure

$X_i$ =mole fraction

With this in mind, we can work with the moles of each compound if we want to analyze the pressure. With the molar mass of each compound we can calculate the moles:

moles of hydrogen gas

The molar mass of hydrogen gas ( $H_2$ ) is 2 g/mol, so:

$6g~H_2\frac{1~mol~H_2}{2~g~H_2}=~3~mol~H_2$

moles of oxygen gas

The molar mass of oxygen gas ( $O_2$ ) is 32 g/mol, so:

$64g~H_2\frac{1~mol~H_2}{32~g~H_2}=~2~mol~O_2$

Now, total moles are:

Total moles = 2 + 3 = 5

With this value, we can write the partial pressure expression for each gas:

$P_H_2=\frac{3}{5}*P_t_o_t_a_l$

$P_O_2=\frac{2}{5}*P_t_o_t_a_l$

So, the answer would be 3/5P.

I hope it helps!

5 0

3 years ago

A solution is prepared from 4.5701 g of magnesium chloride and 43.238 g of water. The vapor pressure of water above this solutio

balandron [24]

Answer:

i = 2.483

Explanation:

The vapour pressure lowering formula is:

Pₐ = Xₐ×P⁰ₐ (1)

For electrolytes:

Pₐ = nH₂O / (nH₂O + inMgCl₂)×P⁰ₐ

Where:

Pₐ is vapor pressure of solution (0.3624atm), nH₂O are moles of water, nMgCl₂ are moles of MgCl₂, i is Van't Hoff Factor, Xₐ is mole fraction of solvent and P⁰ₐ is pressure of pure solvent (0.3804atm)

4.5701g of MgCl₂ are:

4.5701g ₓ (1mol / 95.211g) = 0.048000 moles

43.238g of water are:

43.238g ₓ (1mol / 18.015g) = 2.400 moles

Replacing in (1):

0.3624atm = 2,4mol / (2.4mol + i*0.048mol)×0.3804atm

0.3624atm / 0.3804atm = 2,4mol / (2.4mol + i*0.048mol)

2.4mol + i*0.048mol = 2.4mol / 0.9527

2.4mol + i*0.048mol = 2.5192mol

i*0.048mol = 2.5192mol - 2.4mol

i = 0.1192mol / 0.048mol

i = 2.483

I hope it helps!

4 0

3 years ago