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2 years ago

Why are salt and sugar both able to dissolve in water, even though the solutes have different types of chemical bonding?

Chemistry

1 answer:

Rama09 [41]2 years ago

5 0

Answer:

ions are surrounded by hydrogen ends with positive partial charge. In this way the salt is dissolved in water. Sugar is a molecular compound formed by covalent bonds. In a polar covalent bond, electrons are shared unevenly

Explanation:

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write a balanced chemical equation depicting the formation of one mole of pocl3(l) from its elements in their standard states.

drek231 [11]

Thank you for posting your question here at brainly. Below is the answer:

At 25 C and 1 atm pressure (the standard state): P is a solid, O2 is a gas, and Cl2 is a gas.

P(s) + O2(g) + Cl2(g) ==> POCl3(l) 

To make 1 mole of POCl3, we need to start with 1 mole of P, 1/2 mole of O2, and 3/2 mole of Cl2. 

P(s) + 1/2O2(g) + 3/2Cl2(g) ==> POCl3(l) 

NOTE: Some people write P as P4(s), in which case you would need 1/4 mole P4.

5 0

2 years ago

Read 2 more answers

A 25.0-g sample of ice at -6.5oC is removed from the freezer and allowed to warm until it melts. Given the data below, select al

alukav5142 [94]

Answer:

B, D

Explanation:

The strategy here is to realize that the ice will be taken from -6.5 ºC to OºC where it will melt.

Lets call q₁ the heat required to bring the ice to 0ºc, q₂ the heat required to bring the phase change from solid to liquid.

q₁ is calculated from the expression

q₁ = s x m x ΔT where m is the mass, s the specific heat of ice ( 2.09 J/gºC ) and ΔT the change in temperature.

q₂ the fusion enthalpy change is calculated from the expression:

q₂ = C x ΔT

where C is the specific heat for the phase change , in this case named AH given in kJ/mol.

We are given all the data needed to calculate q₁, q₂ and qtotal ( q₁ + q₂ )

q₁ = 25.0 g x ( 2.09 J/gºC) x ( 0 - ( -6.5 ºC ) )

q₁ = 339.6 J = 0.339 kJ

q₂ = (25 g/ 18 g/mol) x 6.02 kJ/mol = 1.39 x 6.02 kJ = 8.36 kJ

qtotal = 0.339 kJ + 8.36 kJ = 8.70 kJ

with these calculations, we can now proceed to answer the question:

(a) False AH is theheat capacity for the melting.

(b) True as we determined above

(d) True as calculated above

(e) False as determined in our calculations

7 0

1 year ago

A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas reaction vessel. The vessel is

Inessa05 [86]

Answer:

$T=2.78x10^3 \°C$

Explanation:

Hello,

In this case, considering that the safe temperature may be computed via the ideal gas law as we now the pressure, mass and volume via the dimensions:

$V=\pi r^2 h=\pi *(41.0cm)^2*49.2cm=2.60x10^5cm^3*\frac{1L}{1000cm^3} =260L$

The pressure in atm is:

$P=3.70MPa*\frac{1x10^6Pa}{1MPa} \frac{1atm}{101325Pa} =36.5atm$

And the moles considering the mass and molar mass (66 g/mol) of dinitrogen difluoride (N₂F₂):

$n_{N_2F_2}=2.50kg*\frac{1000g}{1kg}*\frac{1mol}{66g} =37.9mol$

In sich a way, by applying the ideal gas equation, which is not the best assumption but could work as an approximation due to the high temperature, the temperature, with three significant figures, will be:

$T=\frac{PV}{nR}=\frac{36.5Pa*260L}{37.9mol*0.082\frac{atm*L}{mol*K} }\\ \\T=3053.6K-273.15\\\\T=2.78x10^3 \°C$