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What can be said about a reaction with H -890 kJmol and S -0.24 kJ(mol K)?
The reaction is exothermic because the enthalpy change is negative (-890 kJ/mol). The reaction may be spontaneous at low temperatures due to the negative entropy change (-0.24 kJ/(mol K)), which decreases the overall spontaneity of the reaction.
What is the value of delta G at 500 K if delta H 27 kJmol and delta S 0.09 kJ(mol K)?
To calculate the value of ΔG at 500 K, you can use the equation ΔG = ΔH - TΔS. Given ΔH = 27 kJ/mol, ΔS = 0.09 kJ/(mol K), and T = 500 K, plug in the values to find ΔG. ΔG = 27 kJ/mol - (500 K)(0.09 kJ/(mol K)) = 27 kJ/mol - 45 kJ/mol = -18 kJ/mol. Therefore, the value of ΔG at 500 K is -18 kJ/mol.
The value of Kb for ammonia is 1.8 x 10-5.Calculate the Gibbs energy change for the base dissociation reaction?
The Gibbs energy change ((\Delta G^\circ)) for the base dissociation reaction of ammonia ((NH_3)) can be calculated using the equation: (\Delta G^\circ = -RT * ln(K_b)) where (K_b) is the base dissociation constant (1.8 x 10^-5) and (R) is the gas constant (8.314 J/mol*K). By substituting the values into the formula, the Gibbs energy change can be calculated.
What does the delta s 0 mean in a reaction?
The delta S^0 in a reaction refers to the standard entropy change. It represents the difference in entropy between the products and reactants at standard conditions (1 atm and 298 K). A positive delta S^0 indicates an increase in disorder or randomness, while a negative delta S^0 indicates a decrease in disorder.
How many grams in 1.90 moles of K?
To convert from moles to grams, we need to use the molar mass of the element. The molar mass of potassium (K) is approximately 39.10 g/mol. So, for 1.90 moles of K, the mass would be 1.90 moles * 39.10 g/mol = 74.29 grams.
How is delta g related to K?
K brings a process including delta g into equilibrium in a reaction. The two work together to maintain a reaction's equilibrium keeping it stable and helping it to continue at a stable rate.
What can be said about a reaction with H -890 kJmol and S -0.24 kJ(mol K)?
The reaction is exothermic because the enthalpy change is negative (-890 kJ/mol). The reaction may be spontaneous at low temperatures due to the negative entropy change (-0.24 kJ/(mol K)), which decreases the overall spontaneity of the reaction.
What is the value of delta G at 500 K if delta H 27 kJmol and delta S 0.09 kJ(mol K)?
To calculate the value of ΔG at 500 K, you can use the equation ΔG = ΔH - TΔS. Given ΔH = 27 kJ/mol, ΔS = 0.09 kJ/(mol K), and T = 500 K, plug in the values to find ΔG. ΔG = 27 kJ/mol - (500 K)(0.09 kJ/(mol K)) = 27 kJ/mol - 45 kJ/mol = -18 kJ/mol. Therefore, the value of ΔG at 500 K is -18 kJ/mol.
Will you trade me a Bakugan?
i will ill swap my 650g delta dragonoid k i will ill swap my 650g delta dragonoid k
At which temperature would a reaction with h-92 kjmol s-0.199 kj(molk) be spontaneous?
To determine whether the reaction is spontaneous, we can use the Gibbs free energy equation, ( \Delta G = \Delta H - T\Delta S ). For the reaction to be spontaneous, ( \Delta G ) must be less than 0. Given ( \Delta H = -92 , \text{kJ/mol} ) and ( \Delta S = -0.199 , \text{kJ/(mol K)} ), we can set up the inequality ( -92 , \text{kJ/mol} - T(-0.199 , \text{kJ/(mol K)}) < 0 ). Solving this will give the temperature threshold above which the reaction becomes spontaneous.
What is negative -k plus negative -k if k equals 2?
neg(-k) + neg(-k) = k + k = 2k = 4
Calculate the specific heat of a substance if 44.0 g of the sample absorbs 67.2 J and the temperature change is 11 K?
The specific heat can be calculated using the formula: ( q = mc\Delta T ), where ( q ) is the heat absorbed, ( m ) is the mass, ( c ) is the specific heat, and ( \Delta T ) is the temperature change. Plugging in the values: ( 67.2 = (44.0) \times c \times 11 ), solving for ( c ) gives a specific heat of approximately 0.138 J/g∙K.
What does linear mean in math definition form?
Definition: An operator L is said to be linearifi) k*L[f] = L[(k*f)]ii) L[f + g] = L[f] + L[g]where k is a constant and f and g are functions.Definition: An equation is said to be linear if it is of the forma1x1 + a2x2 + a3x3 + . . . = 0where a1, a2, a3, . . . are constants and x1, x2, x3, . . . are variables.
The value of Kb for ammonia is 1.8 x 10-5.Calculate the Gibbs energy change for the base dissociation reaction?
The Gibbs energy change ((\Delta G^\circ)) for the base dissociation reaction of ammonia ((NH_3)) can be calculated using the equation: (\Delta G^\circ = -RT * ln(K_b)) where (K_b) is the base dissociation constant (1.8 x 10^-5) and (R) is the gas constant (8.314 J/mol*K). By substituting the values into the formula, the Gibbs energy change can be calculated.
Calculate delta G at 298K for the reaction of nitrogen and hydrogen to form ammonia of the delta G equals -33.3kJn and the reaction mixture consists of the follwing N2.5 atms H2.75 NH3 2.0?
Given that the reaction is N2(g) + 3H2(g) → 2NH3(g), the existing equilibrium constant K at 298K can be calculated using the given partial pressures of N2, H2, and NH3. Then, using the equation ΔG = -RT * ln(K), we can find the Gibbs free energy change. Subtituting the values, we would get ΔG = -33.3kJ/mol.
Is the keyword "k" negative or positive?
The keyword "k" is neutral and does not have a positive or negative connotation.
What does the delta s 0 mean in a reaction?
The delta S^0 in a reaction refers to the standard entropy change. It represents the difference in entropy between the products and reactants at standard conditions (1 atm and 298 K). A positive delta S^0 indicates an increase in disorder or randomness, while a negative delta S^0 indicates a decrease in disorder.
