All categories

3 years ago

The grains of sedimentary rock

Chemistry

1 answer:

Debora [2.8K]3 years ago

3 0

Answer:

The grains of sedimentary rock are cemented together and form an interlocking texture.

Explanation:

The sedimentary rocks are formed by deposition of minerals from the ocean or sea waters lashed to the land shore. The deposition of minerals for a long time followed by cementation of them by the grains lead to the formation of sedimentary rocks.

The grains of the sedimentary rocks are very small in size and they are cemented together. The grains are present in the matrix of cement while the pores of the matrix are filled with grains of minerals like an interlocking texture.

You might be interested in

What family flouride in the table

andrew11 [14]

I assume you're talking about fluorine. Fluorine is in the halogen family and it belongs to group number 17.

6 0

4 years ago

If you combine 230.0 mL 230.0 mL of water at 25.00 ∘ C 25.00 ∘C and 120.0 mL 120.0 mL of water at 95.00 ∘ C, 95.00 ∘C, what is t

Thepotemich [5.8K]

Answer: The final temperature of the mixture is 49°C

Explanation:

To calculate the mass of water, we use the equation:

$\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}$

For cold water:

Density of cold water = 1 g/mL

Volume of cold water = 230.0 mL

Putting values in above equation, we get:

$1g/mL=\frac{\text{Mass of water}}{230.0mL}\\\\\text{Mass of water}=(1g/mL\times 230.0mL)=230g$

For hot water:

Density of hot water = 1 g/mL

Volume of hot water = 120.0 mL

Putting values in above equation, we get:

$1g/mL=\frac{\text{Mass of water}}{120.0mL}\\\\\text{Mass of water}=(1g/mL\times 120.0mL)=120g$

When hot water is mixed with cold water, the amount of heat released by hot water will be equal to the amount of heat absorbed by cold water.

$Heat_{\text{absorbed}}=Heat_{\text{released}}$

The equation used to calculate heat released or absorbed follows:

$Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})$

$m_1\times c\times (T_{final}-T_1)=-[m_2\times c\times (T_{final}-T_2)]$ ......(1)

where,

q = heat absorbed or released

$m_1$ = mass of hot water = 120 g

$m_2$ = mass of cold water = 230 g

$T_{final}$ = final temperature = ?°C

$T_1$ = initial temperature of hot water = 95°C

$T_2$ = initial temperature of cold water = 25°C

c = specific heat of water = 4.186 J/g°C

Putting values in equation 1, we get:

$120\times 4.186\times (T_{final}-95)=-[230\times 4.186\times (T_{final}-25)]$

$T_{final}=49^oC$

Hence, the final temperature of the mixture is 49°C

4 0

4 years ago

A silver chafing dish has a specinc heat capacity of a mass of 1350 How much heat transferred to increase the temperature of by

dezoksy [38]

Answer:

I'm not really sure how to answer it but this is the best I can do:

If the capacity of a mass is 1350 and heat is transferred to increase the temperature by 15. degrees Celcius then the amount of heat that needs to be transferred would be about 45 degrees.

Explanation:

I'm sorry if it's wrong or not exactly the way it's supposed to be answered, I'm not very good with math and temperature problems. But i hope it helps! :)

3 0

3 years ago

A backpacker collects snow at 0°C, and places it in a cooking pot on a camp stove. It takes 643 kJ of heat energy to melt the sn

frutty [35]

Answer:

mass (m) of the snow that the backpacker collected= 0.855 kg

Explanation:

Given that:

Q = 643 kJ = 643000 J

ΔHfusion = 6.02 kJ/mol = 6020 J/mol

number of mole of water H2O = $\frac{mass (m)}{18}$