Is sucrose in water an electrolyte

A solution of ammonia and water contains 2.60×1025 water molecules and 6.90×1024 ammonia molecules. how many total hydrogen atom

marshall27 [118]

1 molecule of NH3 has 3 atoms of H.
6.90*10²⁴ molecules NH3 have 3*6.90*10²⁴ =20.7*10²⁴ atoms H=2.07*10²⁵ atoms H

1 molecule H2O of has 2 atoms of H.
2.60*10²⁵ molecules of H2O have 2*2.60*10²⁵ =5.20 *10²⁵ atoms of H

2.07*10²⁵ + 5.20 *10²⁵ =7.27*10²⁵ atoms of H altogether.

4 0

3 years ago

The atomic mass of titanium is 47.88 atomic mass units. This atomic mass represents the

kkurt [141]

Answer (3) is the most correct, although (2) is not to be ignored. (3) states the most abundant isotope Ti's average mass, which is certainly true. (2) is the total mass of all protons, neutrons, and electrons in an atom of Ti, which is true but has to be more specific in order to pinpoint exactly the 47.88 amu. (4) is incorrect because it is not of all the naturally occurring isotopes of Ti. (1) is incorrect because they forgot electrons.

3 0

3 years ago

Theoretically, how many moles of carbonic acid will be produced by 3.00 g sample of NaHCO3?

Kryger [21]

NaHCO3 = 22.99 + 1.008 + 16(3) = 83.99 g/mol

Na = 22.99g/83.99 g weight of molecule =.2727 or 27.27%

3.0 g* .2727 = 0.8211 grams of sodium in sample of NaHCO3

0.8211 grams Na + 1.266 grams Cl = 2.087 grams

7 0

3 years ago

6. What is the equilibrium constant for the following reaction?<br> C+02 = CO2

Orlov [11]

<h3> $\tt Kc=\dfrac{[CO_2]}{[C][O_2]}$ </h3><h3>Further explanation</h3>

Given

Reaction

C+02 = CO2

Required

The equilibrium constant

Solution

The equilibrium constant is the ratio of concentration or pressure between the product and the reactant with each reaction coefficient raised

The equilibrium constant is based on the concentration (Kc) in a reaction

pA + qB -----> mC + nD

$\large {\boxed {\bold {Kc ~ = ~ \frac {[C] ^ m [D] ^ n} {[A] ^ p [B] ^ q}}}}$

So for the reaction :

C+O₂ ⇔ CO₂

$\tt Kc=\dfrac{[CO_2]}{[C][O_2]}$

8 0

3 years ago

A student dissolves of glucose in of a solvent with a density of . The student notices that the volume of the solvent does not c

nikitadnepr [17]

Answer:

0.052 M

0.059 m

Explanation:

There is some missing info. I think this is the complete question.

<em>A student dissolves 4.6 g of glucose in 500 mL of a solvent with a density of 0.87 g/mL. The student notices that the volume of the solvent does not change when the glucose dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits.</em>

Step 1: Calculate the moles of glucose (solute)

The molar mass of glucose is 180.16 g/mol.

4.6 g × 1 mol/180.16 g = 0.026 mol

Step 2: Calculate the molarity of the solution

0.026 moles of glucose are dissolved in 500 mL (0.500 L) of solution. We will use the definition of molarity.

M = moles of solute / liters of solution

M = 0.026 mol / 0.500 L = 0.052 M

Step 3: Calculate the mass corresponding to 500 mL of the solvent

The solvent has a density of 0.87 g/mL.

500 mL × 0.87 g/mL = 435 g = 0.44 kg

Step 4: Calculate the molality of the solution

We will use the definition of molality.

m = moles of solute / kilograms of solvent

m = 0.026 mol / 0.44 kg = 0.059 m

4 0

3 years ago