How much in mg/l is 0,327 meq/l chloride? I highly appreciate and love to know how you can calculate that.

IrinaVladis [17]

The definition in Volume is a the amount of space a substance or object occupies, or that is enclosed within a container, especially when great. For example "The sewer could not cope with the volume of rainwater" . You can say it in different ways, such as capacity, size, magnitude, mass, bulk, extent and more. I hope this helps :-).

3 0

4 years ago

Consider the reaction.

vovangra [49]

Answer: The value of Keq for the reaction expressed in scientific notation is $1.6\times 10^{-5}$

Explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios.

For the given chemical reaction:

$2NOCl(g)\rightarrow 2NO(g)+Cl_2(g)$

The expression for $K_{eq}$ is written as:

$K_{eq}=\frac{[NO]^2\times [Cl_2]}{[NOCl]^2}$

$K_{eq}=\frac{(1.2\times 10^{-3})^2\times (2.2\times 10^{-3})}{(1.4\times 10^{-2})^2}$

$K_{eq}=1.6\times 10^{-5}$

The value of Keq for the reaction expressed in scientific notation is $1.6\times 10^{-5}$

3 0

3 years ago

A block of iron has a mass of 826 g. What is the volume of the block of iron whose density at 25°C is 7.9

LuckyWell [14K]

Answer:

105

Explanation:

Density = mass/volume

therefore volume = mass/density

826/7.9=105 (To three significant figure)

8 0

3 years ago

According to the following reaction, how much energy is evolved during the reaction of 32.5 g B2H6 with excess Cl2? The molar ma

bonufazy [111]

Answer:

1640 kJ are involved in the reaction

Explanation:

In the reaction:

B₂H₆(g) + 6Cl₂(g) → 2 BCl₃(g) + 6HCl(g)

1 mol of B₂H₆(g) with 6 moles of Cl₂(g) produce 1396 kJ of energy.

Now if 32.5g of B₂H₆(g) react with excess Cl₂(g), moles involved in reaction are:

$32.5g B_2H_6\frac{1mol}{27.67g} = 1.175 moles$

If 1 mol produce 1396kJ of energy, 1.175 moles produce:

$1.175mol\frac{1396kJ}{1mol} = 1640kJ\\$

Thus, 1640 kJ are involved in the reaction

5 0

4 years ago

Read 2 more answers

A chemistry student needs 60.0 ml of ethanolamine for an experiment. By consulting the CRC Handbook of Chemistry and Physics, th

BARSIC [14]

Answer:

The student should weigh out 61.2g of ethanolamine [6.12 * 10]

Explanation:

In this question, we are expected to calculate the mass of ethanolamine needed to make 60.0ml of it given that the density of the ethanolamine in question is 1.02g/cm^3

Mathematically, it has been shown that mass = density * volume

Hence, by multiplying the density by the volume, we get the mass.

Now, from the question we can see that we have the values for the density and the volume. We now need to get the mass.

Since cm^3 is same as ml, we need not perform any conversion.

Hence, the needed mass is:

60 * 1.02 = 61.2g

6 0

4 years ago