All categories

2 years ago

How many grams of water would there be in 100.0g of hydrate? How many moles?

2 answers:

7 0

<u>Answer:</u> The mass of water present in given amount of hydrate is 36.68 grams and number of moles of water are 2.04 moles.

<u>Explanation:</u>

We are given:

Mass of hydrate = 0.946 grams

Mass of water present = 0.347 grams

We need to calculate the mass of water present in 100 grams of hydrate. By using unitary method, we get:

In 0.946 g of hydrate, the amount of water present is 0.347 g

So, in 100 g of hydrate, the amount of water present will be = $\frac{0.347g}{0.946g}\times 100g=36.68g$

Hence, the mass of water present in given amount of hydrate is 36.68 grams.

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of water = 36.68 g

Molar mass of water = 18 g/mol

Putting values in above equation, we get:

$\text{Moles of water}=\frac{36.38g}{18g/mol}=2.04mol$

Hence, the number of moles of water are 2.04 moles.

IceJOKER [234]2 years ago

6 0

The calculation for the amount of water present in the given amount of hydrate is shown below,
amount water = (100 g hydrate) x (0.347 g H2O / 0.946 g hydrate)
= 36.68 g
Thus, the amount of water present in the hydrate is approximately 36.68 g.

You might be interested in

Using only the following elements P, Br, and Mg, give the formulas for:A. an ionic compound. B. a molecular compound with polar

Talja [164]

Answer:

<h2>1. Ionic compound- $MgBr_2$ </h2><h2>2. Polar molecular compound- $PBr_3$ </h2>

Explanation:

Mg is a metal that has 12 atomic numbers and thus its electronic configuration is $1s^22s^22p^63s^2$ . The outer most shell of this element has 2 electrons so it loses 2 electrons and thus form $Mg^2^+$ ions. Br is a nonmetal and has 35 atomic number so its electronic configuration is $1s^22s^22p^63s^23p^64s^23d^1^04p^5$ . Since its outermost shell has 7 electrons so it can accept one electron and thus forms $Br^-$ . So magnesium ion and bromide ion combine and forms an ionic compound $MgBr_2$ .

P is also a nonmetal and combine with Br with covalent bond and due to electronegativity differences form polar covalent compound such as $PBr_3$ .

8 0

1 year ago

The temperature at the boiling point remained constant despite the continued addition of heat by the bunsen burner. What was the

Paul [167]

Concept:

<em><u>Latent Heat of Vaporization</u></em>: It is defined as the amount of heat required to change the state of mater without changing of its temperature.

From the given question, the temperature at the boiling point remained constant despite the continued addition of heat by the Bunsen burner. <em>Actually,</em> this amount of heat is used by water to break the intermolecular bonds between the water molecules in the form of latent heat that converts the liquid state of water into vapor state of water.

Hence, the correct option will be d.<u>The energy was used to break the intermolecular bonds between the water molecules. </u>

3 0

2 years ago

Under standard conditions, a given reaction is endergonic (i.e., ΔG >0). Which of the following can render this reaction favo

sleet_krkn [62]

Answer:

Maintaining a high starting-material concentration can render this reaction favorable.

Explanation:

A reaction is <em>favorable</em> when <em>ΔG < 0</em> (<em>exergonic</em>). ΔG depends on the temperature and on the reaction of reactants and products as established in the following expression:

ΔG = ΔG° + R.T.lnQ

where,

ΔG° is the standard Gibbs free energy

R is the ideal gas constant

T is the absolute temperature

Q is the reaction quotient

To make ΔG < 0 when ΔG° > 0 we need to make the term R.T.lnQ < 0. Since T is always positive we need lnQ to be negative, what happens when Q < 1. Q < 1 implies the concentration of reactants being greater than the concentration of products, that is, maintaining a high starting-material concentration will make Q < 1.

5 0

1 year ago

What is the millimolar solubility of oxygen gas, o2, in water at 16 ∘c, if the pressure of oxygen is 1.00 atm?

Artyom0805 [142]

Partial pressure is the amount of pressure or force that is exerted by the atoms into the outer environment. it is dependent on the temperature and pressure of the present surroundings. in this case, we are asked in this problem to determine the partial pressure of oxygen at 16oC and 1 atm. We have to look into a solubility data table commonly found in handbooks and determined via experiments and correlations. According to literature, the value of the partial pressure is equal to 0.617 mM.This is under the assumption that the salinity of the water in which oxygen is dissolved is equal to zero.

8 0

1 year ago

Read 2 more answers

Calculate the Lattice Energy of KCl(s) given the following data using the Born-Haber cycle: ΔHsublimation K = 79.2 kJ/mol IE1 K

DanielleElmas [232]

Answer:

Explanation:

The following equation relates to Born-Haber cycle

$\triangle H_f = S + \frac{1}{2} B + IE_M - EA_X+ U_L$