heating a sample of water from -20∘c to 130∘c will involve a calculation that includes how many steps? select the correct answer below: 5 4 3 2

Answers

Answer 1

A sample of water from -20∘C to 130∘C involves four steps: heating the sample from -20∘C to 0∘C, melting the sample at 0∘C, heating the sample from 0∘C to 100∘C, and finally, boiling the sample at 100∘C.

The calculation of heating a sample of water from -20∘C to 130∘C involves four steps.

These steps include heating the sample from -20∘C to 0∘C, melting the sample at 0∘C, heating the sample from 0∘C to 100∘C, and finally, boiling the sample at 100∘C.

Heating the sample from -20∘C to 0∘C, Melting the sample at 0∘C, Heating the sample from 0∘C to 100∘C, and Boiling the sample at 100∘C. The water experiences phase changes at 0∘C and 100∘C. These phase changes involve absorbing or releasing heat energy, but the temperature does not change during these phase changes. During the steps where the temperature is increasing, the heat energy absorbed by the water can be calculated using the specific heat capacity of water.

The summary of the answer is that the calculation of heating a sample of water from -20∘C to 130∘C involves four steps: heating the sample from -20∘C to 0∘C, melting the sample at 0∘C, heating the sample from 0∘C to 100∘C, and finally, boiling the sample at 100∘C.

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Related Questions

if the density of an unknown gas is 1.96 g/l at stp, what is its molar mass?

Answers

The molar mass of the unknown gas is approximately 43.68 g/mol.

To determine the molar mass of the unknown gas, we can use the ideal gas law equation, which states:

PV = nRT

Where:

P is the pressure (in this case, at STP, it is 1 atm)

V is the volume (given as 1 L)

n is the number of moles of the gas

R is the ideal gas constant (0.0821 L·atm/(mol·K))

T is the temperature in Kelvin (273.15 K at STP)

Rearranging the equation, we have:

n = PV / RT

Substituting the given values, we get:

n = (1 atm) * (1 L) / (0.0821 L·atm/(mol·K) * 273.15 K)

n = 0.04489 mol

To determine the molar mass, we divide the mass of the gas by the number of moles:

Molar mass = Mass / n

Given the density of the gas as 1.96 g/L, the mass of 1 L of the gas is 1.96 g.

Molar mass = 1.96 g / 0.04489 mol

Molar mass = 43.68 g/mol

Therefore, the molar mass of the unknown gas is approximately 43.68 g/mol.

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the diffusion coefficient of fe in bcc iron is approximately 3 x 10-11 cm2/s at 900 oc and 1.5 x 10-14 cm2/s at 630oc. the activation energy in cal/mol is approximately

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The activation energy of Fe in BCC iron is approximately 139.06 cal/mol at 900 OC and 199.17 cal/mol at 630 OC.

Given:The diffusion coefficient of Fe in BCC iron is approximately 3 x 10-11 cm2/s at 900 OC and 1.5 x 10-14 cm2/s at 630OCFormula:The Arrhenius equation: k = Ae^(-Q/RT)

Activation Energy, Q = -R ln(k/T)where R is the gas constant, k is the rate constant, T is the absolute temperature, and A is the pre-exponential factor.Calculation:R = 1.987 cal/(mol K)

The activation energy is given byQ=−Rln(kT)At 900 OC: k= 3 x 10-11 cm2/s and T = 1173 KR= 1.987 cal/mol.Kln(kT) = ln(3 x 10^-11 cm²/s × 1173 K) = -69.91 Q = -1.987 cal/(mol K) × (-69.91) Q = 139.06 cal/molAt 630 OC: k = 1.5 × 10-14 cm2/s and T = 903 KR = 1.987 cal/(mol K)ln(kT) = ln(1.5 × 10^-14 cm²/s × 903 K) = -100.32 Q = -1.987 cal/(mol K) × (-100.32) Q = 199.17 cal/mol

Therefore, the activation energy of Fe in BCC iron is approximately 139.06 cal/mol at 900 OC and 199.17 cal/mol at 630 OC.

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ammonia is a weak base that will react in water following the equation below. nh3 h2o⟶x oh− what is the chemical formula for the conjugate acid of nh3?

Answers

Ammonia (NH₃) being a weak base, accepts the hydrogen ion from water to form its conjugate acid, ammonium (NH₄⁺).

Ammonia (NH₃) is a weak base that reacts with water (H₂O) to form its conjugate acid and a hydroxide ion (OH⁻) in the process called acid-base reaction. When NH₃ interacts with H₂O, a hydrogen ion (H⁺) from water is transferred to ammonia, resulting in the formation of the conjugate acid of NH₃, which is ammonium (NH₄⁺). At the same time, the hydroxide ion (OH⁻) is produced as a byproduct. The overall balanced equation for this reaction is:

NH₃ (aq) + H₂O (l) ⟶ NH₄⁺ (aq) + OH⁻ (aq)

Here, the chemical formula for the conjugate acid of ammonia (NH₃) is NH₄⁺. It is essential to understand that a conjugate acid is formed when a base accepts a hydrogen ion (H⁺) from the reacting species. In this case, ammonia (NH₃) being a weak base, accepts the hydrogen ion from water to form its conjugate acid, ammonium (NH₄⁺).

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