How many molecules are their in o.5 mole of H2o

This is the SI unit for force meter liter Newton m/s/s

morpeh [17]

The newton is the SI unit for force; it is equal to the amount of net force required to accelerate a mass of one kilogram at a rate of one meter per second squared. Newton's second law of motion states: F = ma, multiplying m (kg) by a (m/s 2 ).

I don't understand your question, but I think that would help.

4 0

3 years ago

A certain chemical reaction releases 36.2 kJ/g of heat for each gram of reactant consumed. How can you calculate what mass of re

Lilit [14]

Answer:

0.038 g of reactant

Explanation:

Data given:

Heat release for each gram of reactant consumption = 36.2 kJ/g

mass of reactant that release 1360 J of heat = ?

Solution:

As 36.2 kJ of heat release per gram of reactant consumption so first we will convert KJ to J

As we know

1 KJ = 1000 J

So

36.2 kJ = 36.2 x 1000 = 36200 J

So it means that in chemical reaction 36200 J of heat release for each gram of reactant consumed so how much mass of reactant will be consumed if 1360 J heat will release

Apply unity formula

36200 J of heat release ≅ 1 gram of reactant

1360 J of heat release ≅ X gram of reactant

Do cross multiplication

X gram of reactant = 1 g x 1360 J / 36200 J

X gram of reactant = 0.038 g

So 0.038 g of reactant will produce 1360 J of heat.

5 0

2 years ago

In a living organism, what is an organ? functional unit, or building block, of all organisms; smallest unit that can carry on th

ra1l [238]

Answer: D. a structure that provides a specific service within a cell

Explanation:

7 0

2 years ago

onsider the following reaction: CaCN2 + 3 H2O → CaCO3 + 2 NH3 105.0 g CaCN2 and 78.0 g H2O are reacted. Assuming 100% efficiency

mestny [16]

Answer : The excess reactant is, $H_2O$

The leftover amount of excess reagent is, 7.2 grams.

Solution : Given,

Mass of $CaCN_2$ = 105.0 g

Mass of $H_2O$ = 78.0 g

Molar mass of $CaCN_2$ = 80.11 g/mole

Molar mass of $H_2O$ = 18 g/mole

Molar mass of $CaCO_3$ = 100.09 g/mole

First we have to calculate the moles of $CaCN_2$ and $H_2O$ .

$\text{ Moles of }CaCN_2=\frac{\text{ Mass of }CaCN_2}{\text{ Molar mass of }CaCN_2}=\frac{105.0g}{80.11g/mole}=1.31moles$

$\text{ Moles of }H_2O=\frac{\text{ Mass of }H_2O}{\text{ Molar mass of }H_2O}=\frac{78.0g}{18g/mole}=4.33moles$

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

$CaCN_2+3H_2O\rightarrow CaCO_3+2NH_3$

From the balanced reaction we conclude that

As, 1 mole of $CaCN_2$ react with 3 mole of $H_2O$

So, 1.31 moles of $CaCN_2$ react with $1.31\times 3=3.93$ moles of $H_2O$

From this we conclude that, $H_2O$ is an excess reagent because the given moles are greater than the required moles and $CaCN_2$ is a limiting reagent and it limits the formation of product.

Left moles of excess reactant = 4.33 - 3.93 = 0.4 moles

Now we have to calculate the mass of excess reactant.

$\text{ Mass of excess reactant}=\text{ Moles of excess reactant}\times \text{ Molar mass of excess reactant}(H_2O)$

$\text{ Mass of excess reactant}=(0.4moles)\times (18g/mole)=7.2g$

Thus, the leftover amount of excess reagent is, 7.2 grams.

8 0

3 years ago

The enzyme urease catalyzes the breakdown of urea in the body. Urease breaks urea down to 2NH3+CO2. This is an example of a hydr

Alika [10]

Answer:

Look at the picture.

Explanation:

On stage one binding of a substrate occurs (and also the geometry of active site may change) and water comes to the site. On stage two the hydrolisis takes place and on stage 3 products deabsorb from the enzyme.

8 0

2 years ago